Question Bank › Physical Chemistry › Elementary Process Rate Constant › ABC26PH1034ABC26PH1034 · Elementary Process Rate Constant Subject: Physical Chemistry · Chapter: Elementary Process Rate Constant · Topic: Elementary Process Rate Constant – General · Exam: NET DEC 2019 · Marks: 2 · Difficulty: Hard
The oxidation of NO to $\mathrm{NO}_{2}$ occurs via the mechanism given below \[ \begin{array}{l} 2\mathrm{NO} \underset{k_{-1}}{\overset{k_{1}}{\rightleftharpoons}} \mathrm{N_2O_2} \\ \mathrm{N_2O_2 + O_2} \xrightarrow{k_{2}} 2\mathrm{NO_2} \end{array} \]
$\frac{\mathrm{d}\left[\mathrm{NO}_{2}\right]}{\mathrm{dt}}$ in the presence of large excess of $\mathrm{O}_{2}$ can be written as (a) $2 \mathrm{k}_{1}(\mathrm{NO})_{2}$
(b) $2 \mathrm{k}_{1} \mathrm{k}_{2}(\mathrm{NO})_{2}\left(\mathrm{O}_{2}\right)$
(c) $\frac{\mathrm{k}_{1}}{\mathrm{k}_{2}}(\mathrm{NO})^{2}$
(d) $2 \mathrm{k}_{2}(\mathrm{NO})^{2}$
Answer SELF-PRACTICE — the source book printed no answer.
Nothing is invented here, so this question has no answer on record.
Explanation No explanation was printed for this question.
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